Ch.7 - Quantum MechanicsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Calculate the wavelength of light that would cause an electron to transition from  n = 1 to n = 3 in the hydrogen atom. A) 103 nm B) 136 nm C) 646 nm D) 155 nm E) 971 nm

Problem

Calculate the wavelength of light that would cause an electron to transition from  n = 1 to n = 3 in the hydrogen atom.

 A) 103 nm 

B) 136 nm 

C) 646 nm 

D) 155 nm 

E) 971 nm

Solution

We are asked to calculate the wavelength of light that would make an electron transition from n=1 to n=3. 


For this problem we would use the Balmer equation: 

1λ= R1nf2 - 1ni2

Where:

λ = wavelength (m)
R = 1.0974 x 107 m-1
nf = final energy level
ni = intial energy level

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